sing the general properties of equilibrium cor a certain temperature, the equilibrium constant for the following reaction is 5.41 x 10 NO₂(g) + CO(g) NO(g) + CO₂(g) se this information to complete the following table. 1 Suppose a 47. L reaction vessel is filled with 0.56 mol of NO₂ and 0.56 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 3 NO₂(g) +3CO(g) 3 NO(g) + 3C0₂(a) O There will be very little NO₂ and Co. O There will be very little NO and CO₂ ONeither of the above is true. K=O K-O

sing the general properties of equilibrium cor a certain temperature, the equilibrium constant for the following reaction is 5.41 x 10 NO₂(g) + CO(g) NO(g) + CO₂(g) se this information to complete the following table. 1 Suppose a 47. L reaction vessel is filled with 0.56 mol of NO₂ and 0.56 mol of CO. What can you say about the composition of the mixture in the vessel at equilibrium? What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. NO(g) + CO₂(g) NO₂(g) +CO(g) What is the equilibrium constant for the following reaction? Be sure your answer has the correct number of significant digits. 3 NO₂(g) +3CO(g) 3 NO(g) + 3C0₂(a) O There will be very little NO₂ and Co. O There will be very little NO and CO₂ ONeither of the above is true. K=O K-O

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 123CP: A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless,...

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Two molecules of A react to form one molecule of B, as in the reaction 2 A(g) B(g) Three experiments are done at different temperatures and equilibrium concentrations are measured. For each experiment, calculate the equilibrium constant, Kc. (a) [A] = 0.74 mol/L, [B] = 0.74 mol/L (b) [A] = 2.0 mol/L, [B] = 2.0 mol/L (c) [A] = 0.01 mol/L, [B] = 0.01 mol/L What can you conclude about this statement: If the concentrations of reactants and products are equal, then the equilibrium constant is always 1.0.
You place 0.600 mol of nitrogen, N2, and 1.800 mol of hydrogen, H2, into a reaction vessel at 450C and 10.0 atm. The reaction is N2(g)+3H2(g)2NH3(g) What is the composition of the equilibrium mixture if you obtain 0.048 mol of ammonia, NH3, from it?
At 25C. Kp = 5.3 105 for the reaction N2(g)+3H2(g)2NH3(g) When a certain partial pressure of NH3(g) is put into an otherwise empty rigid vessel at 25C, equilibrium is reached when 50.0% of the original ammonia has decomposed. What was the original partial pressure of ammonia before any decomposition occurred?
Consider the equilibrium N2(g)+O2(g)2NO(g) At 2300 K the equilibrium constant Kc = 1.7 103. If 0.15 mol NO(g) is placed into an empty, sealed 10.0-L flask and heated to 2300 K, calculate the equilibrium concentrations of all three substances at this temperature.
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L"' ofO2, what were the equilibrium concentrations of all species?
12.101 An engineer working on a design to extract petroleum from a deep thermal reservoir wishes to capture toxic hydrogen sulfide gases present by reaction with aqueous iron(II) nitrate to form solid iron(II) sulfide. (a) Write the chemical equation for this process, assuming that it reaches equilibrium. (b) What is the equilibrium constant expression for this system? (c) How can the process be manipulated so that it does not reach equilibrium, allowing the continuous removal of hydrogen sulfide?
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?

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